WORK, HEAT, HEAT ENGININES

1. Thermodynamics
Temperature, Heat, Work
Heat Engines

2. Introduction
 In mechanics we deal with quantities such
as mass, position, velocity, acceleration,
energy, momentum, etc.
 Question: What happens to the energy of
a ball when we drop it on the floor?
 Answer: It goes into heat energy.
 Question: What is heat energy?

3. The answer is a bit longer.
 In Thermodynamics we deal with
quantities which describe our system,
usually (but not always) a gas.
 Volume, Temperature, Pressure, Heat
Energy, Work.

4.  We all know about Volume.
 Pressure:
Area
Force
Pressure
Demonstrations: Balloons, Bed of Nails, Magdeburg hemispheres.

5. Example
 120 lb woman putting all her weight on
2in2 of heals.
 Pressure = 120 lb/2in2 = 60 lb/in2.
 Is that a lot?
 Comparison: 1 atm = 14.7 lb/in2. Thus of
heals is approximately 4 atm.
 This is the pressure you would feel at a
depth of approximately 133 ft of water.

6. Temperature and Heat
 Everyone has a qualitative understanding
of temperature, but it is not very exact.
 Question: Why can you put your hand in a
400 F oven and not get instantly burned,
but if you touch the metal rack, you do?
 Answer: Even though the air and the rack
are at the same temperature, they have
very different energy contents.

7. Construction of a Temperature Scale
 Choose fixed point temperatures that are easy
to reconstruct in any lab, e.g. freezing point of
water, boiling point of water, or anything else
you can think of.
 Fahrenheit: Original idea:
0F Freezing point of Salt/ice
100FBody Temperature
Using this ice melts at 32F and water boils at
212F (Not overly convenient) Note: 180F
between boiling an freezing.

8.  Celsius (Centigrade) Scale:
0C Ice Melts
100C Water Boils
Note a change of 1C = a change of 1.8F.

9. Conversion between Fahrenheit
and Celsius
 
32
9
5
C
Celsius
want
and
Fahrenheit
know
we
If
32
5
9
Fahrenheit
want
and
Celsius
know
we
If




F
C
F

10. Absolute or Kelvin Scale
 The lowest possible temperature on the
Celsius Scale is -273C.
 The Kelvin Scale just takes this value and
calls it 0K, or absolute zero.
 Note: the “size” of 1K is the same as 1C.
 To convert from C to K just add 273.
K=C+273

11. When do you use which scale.
 Never use Fahrenheit, except for the
weather.
 You can always use Kelvin and you must
use Kelvin when doing absolute
temperature measurements.
 You can use either Kelvin or Celsius when
measuring differences in temperature.

12. Heat
 Heat is the random
motion of the particles
in the gas, i.e. a
“degraded” from of
kinetic energy.
 Nice web simulation
 gas simulation

13.  The higher the temperature, the faster the
particles (atoms/molecules) are moving,
i.e. more Kinetic Energy.
 We will take heat to mean the thermal
energy in a body OR the thermal energy
transferred into/out of a body

14. Specific Heat
 Observational Fact: It is easy to change the temperature
of some things (e.g. air) and hard to change the
temperature of others (e.g. water)
 The amount of heat (Q) added into a body of mass m to
change its temperature an amount T is given by
Q=m C T
 C is called the specific heat and depends on the
material and the units used.
 Note: since we are looking at changes in
temperature, either Kelvin or Celsius will do.

15. Units of Heat
 Heat is a form of energy so we can always
use Joules.
 More common in thermodynamics is the
calorie: By definition 1 calorie is the
amount of heat required to change the
temperature of 1 gram of water 1C.
 1 Cal = 1 food calorie = 1000 cal.

16.  The English unit of heat is the Btu (British
Thermal Unit.) It is the amount of heat
required to change the temperature of 1
lb of water 1F.
 Conversions:
1 cal =4.186 J
1Btu = 252 cal

17. Units of Specific Heat




















C
kg
J
C
g
cal
T
m
Q
C o
o
Note that by definition, the specific
heat of water is 1 cal/gC.

18. Material J/kgC cal/gC
Water 4186 1
Ice 2090 0.50
Steam 2010 0.48
Silver 234 0.056
Aluminum 900 0.215
Copper 387 0.0924
Gold 129 0.0308
Iron 448 0.107
Lead 128 0.0305
Brass 380 0.092
Glass 837 0.200
Wood 1700 0.41
Ethyl Alcohol 2400 0.58
Beryllium 1830 0.436

19. Water has a specific heat of 1 cal/gmK and iron has
a specific heat of 0.107 cal/gmK. If we add the
same amount of heat to equal masses of iron and
water, which will have the larger change in
temperature?
1. The iron.
2. They will have equal
changes since the same
amount of heat is added
to each.
3. The Water.
4. None of the above.

20. Example Calculation
 Compare the amount of heat energy required to
raise the temperature of 1 kg of water and 1 kg
of iron 20 C?
cal
C
C
g
cal
g)
(
Q
cal
C
C
g
cal
g)
(
Q
T
mC
Q
o
o
o
o
2140
)
20
)(
/
107
.
0
(
1000
Iron
For
000
,
20
)
20
)(
/
1
(
1000
For Water







21. Heat Transfer Mechanisms
1. Conduction: (solids--mostly) Heat
transfer without mass transfer.
2. Convection: (liquids/gas) Heat transfer
with mass transfer.
3. Radiation: Takes place even in a
vacuum.

22. Conduction
 
T
d
A
t
Q




























Thickness
Difference
e
Temperatur
Area
Contact
ty
Conductivi
Thermal
Flow
Heat
of
Rate

24. Example

25. Convection
 Typically very
complicated.
 Very efficient way to
transfer energy.
 Vortex formation is
very common feature.
 liquid convection
 vortex formation
 Sunspot
 solar simulation

26. Convection Examples
 Ocean Currents

27.  Plate tectonics

28. Radiation
 Everything that has a temperature
radiates energy.
 Method that energy from sun reaches
the earth.
4
4
)
( T
const
eAT
t
Q
P 

 

29.  Note: if we double the temperature, the
power radiated goes up by 24 =16.
 If we triple the temperature, the radiated
power goes up by 34=81.
 A lot more about radiation when we get to
light.

31. Work Done by a Gas
 Work=(Force)x(distance)
=Fy
 Force=(Presssure)x(Area)
 W=P(Ay)
=PV

32. First Law of Thermodynamics
Conservation of energy
 When heat is added into a system it can
either 1) change the internal energy of the
system (i.e. make it hotter) or 2) go into
doing work.
Q=W +U.
Note: For our purposes, Internal Energy is the part
of the energy that depends on Temperature.

33. Heat Engines
 If we can create an “engine” that
operates in a cycle, we return to our
starting point each time and therefore
have the same internal energy. Thus,
for a complete cycle
Q=W

34. Model Heat Engine
 Qhot= W+Qcold
or
 Qhot-Qcold=W
(what goes in must
come out)

35. Efficiency
 We want to write an expression that
describes how well our heat engine works.
 Qhot=energy that you pay for.
 W=work done (what you want.)
 Qcold= Waste energy (money).
Efficiency = e = W/Qhot

36.  If we had a perfect engine, all of the input heat
would be converted into work and the efficiency
would be 1.
 The worst possible engine is one that does no
work and the efficiency would be zero.
 Real engines are between 0 and 1
hot
cold
hot
cold
hot
hot Q
Q
Q
Q
Q
Q
W
e 



 1

37. Newcomen Engine
(First real steam engine)
e=0.005

38. Example Calculation
 In every cycle, a heat engine absorbs
1000 J from a hot reservoir at 600K, does
400 J of work and expels 600 J into a cold
reservoir at 300K. Calculate the efficiency
of the engine.
 e= 400J/1000J=0.4
 This is actually a pretty good engine.

39. Second Law of Thermodynamics
(What can actually happen)
 Heat does not voluntarily flow from cold to
hot.
OR
 All heat engines have e<1. (Not all heat
can be converted into work.)

40. Carnot Engine
 The very best theoretically possible heat
engine is the Carnot engine.
 The efficiency of a Carnot engine depends
on the temperature of the hot and cold
reservoirs.
!
!
Kelvins!
in
measured
be
must
res
temperatu
The
:
Note
1
hot
cold
Carnot
T
T
e 


41. Example Calculation Part II
 In every cycle, a heat engine absorbs
1000 J from a hot reservoir at 600K, does
400 J of work and expels 600 J into a cold
reservoir at 300 K. Calculate the
efficiency of the best possible engine.
 e= 1-300/600 =0.5
 Recall that the actual engine has e=0.4.